Question

The ideal gas equation holds for all ideal gases despite them moving at different speeds. A concept
also known as “Avogadro’s hypothesis”.
I. How much faster on average does H2 travel than O2?
II. Given that at the same n, T, and V these two gases have the same P, what can you say about
the average force exerted on the walls of the container with each collision for O2 versus H2?
III. In one sentence, describe the differences in the molecular origin of P in O2 versus H2.

Answer 1

Hello,
The gases differ because all the distinguishing characteristics are provided by the electronegativity, the density, the molecular weight, the distribution of the molecule among other things, understanding that, then:

I. Oxygen and hydrogen differ by density. The less dense element diffuses more rapidly to the surrounding medium. Oxygen with a density of 1.429 g / l, is much higher than 0.071 g / l, value of hydrogen, so this means that the rate of diffusion of hydrogen is greater than that of oxygen.

II. Both gases are in the same starting point, but because oxygen has a higher molecular weight than hydrogen, 32 and 1, respectively, indicates that oxygen will need more space, that is, more volume inside a container, so the force exerted by the oxygen is greater than the force by the hydrogen gas.

III. The oxygen molecule is larger with greater presence of orbitals to the hydrogen molecule, producing higher pressure.